A molecule can either be polar or non-polar depending on whether the molecule has an even distribution of electrons or not.
A polar molecule does not have an even distribution of electrons. The electrical charges are not evenly distributed, causing one end to be more charged than the other.
A non-polar molecule has an even distribution of electrons. Since the electrical charges are evenly distributed, they cancel each other out.

Chloroform can be written as CHCl3.
Therefore the Lewis Structure of Chloroform is:

As you can see, there are four bonds in CHCl3 but two different bonds: C-H and C-Cl

Finding the electronegativity value of each atom in the bond can help determine the energy flow and whether a molecule is polar or non-polar.

(green = Cl, black = C, white = H)

According to the Electronegativity Table, the electronegativity values of the atoms in CHCl3 are:
C - 2.5
H - 2.2
Cl - 3.2
In the picture below, the arrows represent the energy flow of each bond, for it goes from lower value to higher value.
So the arrow goes from H (2.2) to C (2.5)
and from C (2.5) to Cl (3.2)
If the arrows all point to the same central atom, or if the arrows cancel each other out, then the molecule is non-polar, if not, than the molecule is polar.

The arrows do not cancel each other out, for Cl is more negatively charged than C and H. Therefore Chloroform is a polar molecule because it does not have an even distribution of molecules, and one end is more negatively charged (Cl) than another (H).

London Dispersion forces occur between all molecules for they are weak temporary forces that attract two molecules when two atoms adjacent to each other have electrons in positions that cause the atoms to form temporary dipoles.

Dipole-Dipole Forces

Dipole Dipole forces only occur between polar molecules, for they are forces that attract the positive end of one molecule to the negative end of another adjacent molecule.

Hydrogen Bonding

Hydrogen Bonding only occurs in some polar molecules, for they are a type of dipole-dipole forces. Hydrogen bonding is a force that attracts the hydrogen of one molecule to the Nitrogen, Oxygen, or Fluorine of an adjacent molecule.

Chloroform (CHCl3) uses London Dispersion Forces and Dipole-Dipole Forces to attract with another identical molecule, as shown in the picture below. *Note that the London Dispersion forces could not be showed because they are constantly forming all around the molecule, changing places.

Chloroform uses London Dispersion Forces because all molecules regardless of polarity use them. Chloroform additionally uses Dipole-Dipole Forces because it is polar, and only polar molecules exhibit Dipole-Dipole forces, for polar molecules have oppositely charged ends that attract each other, while a non-polar molecule does not. Chloroform does not use Hydrogen Bonding because it does not contain any Nitrogen, Oxygen, or Fluorine that the Hydrogen can bond to.